Consider the titration of 35.0 mL of 0.260 M HF with 0.215 MNaOH. Calculate the pH...

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Chemistry

Consider the titration of 35.0 mL of 0.260 M HF with 0.215MNaOH. Calculate the pH at each of the following points.
Part A.)
How many milliliters of base are required to reach theequivalence point?
Express your answer using three significant figures.
Part B.)
Calculate the pH after the addition of 8.75 mL of base
Express your answer using two decimal places.
Part C.)
Calculate the pH at halfway to the equivalence point.
Express your answer using two decimal places.
Part D.)
Calculate the pH at the equivalence point.
Express your answer using two decimal places.
Part E.)
Calculate the pH after the addition of 70.0 mL of base.
Express your answer using two decimal places.

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Consider the titration of 350 mL of 0260 M HF with 0215 MNaOH Calculate the pH at each of the following points Part A How many milliliters of base are required to reach the equivalence point Express your answer using three significant figures Reaction of HF and NaOH HF NaOH NaF H2O Moles of HF 0035 L 0260 M 91103 mol HF Moles of NaOH 91103 mol because 1 See Answer

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